In the breakdown of a compound into its constituent parts, the generalized reaction for chemical decomposition is: : ( represents the reactant that begins the reaction, and and represent the products of the reaction) An example is the
electrolysis of water to the gases hydrogen and oxygen: :
Additional examples An example of a catalytic decomposition is that of
hydrogen peroxide with a catalytic amount of
manganese dioxide () added, which causes an extremely rapid decomposition to oxygen and water: : This reaction is one of the exceptions to the endothermic nature of decomposition reactions. Other reactions involving decomposition do require the input of external energy. This energy can be in the form of heat, radiation, electricity, or light. The latter being the reason some chemical compounds, such as many prescription medicines, are kept and stored in dark bottles which reduce or eliminate the possibility of light reaching them and initiating decomposition. When heated,
carbonates will decompose.
Carbonic acid (), commonly seen as the "fizz" in carbonated beverages, will spontaneously decompose over time into
carbon dioxide and water over time without external heat: : Other carbonates will decompose when heated to produce their corresponding
metal oxide and carbon dioxide. The following equation is an example, where represents the given metal: : A specific example is that involving
calcium carbonate: : Metal
chlorates also decompose when heated. In this type of decomposition reaction, a metal
chloride and oxygen gas are the products. Here, again, represents the metal: : A common decomposition of a chlorate is in the reaction of
potassium chlorate where oxygen is the product. This can be written as: : ==See also==